Why diamond is a non-conductor while graphite is a conductor?

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SECTION - I

Q#2: Give Short Answers to the following questions. (Any EIGHT)

1. Why diamond is a non-conductor while graphite is conductor?
   • In diamond, each carbon atom is sp$^3$ hybridized and forms four strong sigma bonds with other carbon atoms. All valence electrons are localized in these bonds, so there are no free electrons to conduct electricity.
   • In graphite, each carbon atom is sp$^2$ hybridized and forms three sigma bonds. The remaining unhybridized p-orbitals overlap to form a delocalized pi electron cloud above and below the planes. These delocalized electrons are free to move, making graphite a good electrical